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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblem 39b
Chapter 4, Problem 39b

Consider the reaction: 4 HCl(g) + O2(g) → 2 H2O(g) + 2 Cl2(g) Each molecular diagram represents an initial mixture of reactants. How many molecules of Cl2 form from the reaction mixture that produces the greatest amount of products?

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Identify the balanced chemical equation: 4 \(\text{HCl}\)(g) + \(\text{O}\)_2(g) \(\rightarrow\) 2 \(\text{H}\)_2\(\text{O}\)(g) + 2 \(\text{Cl}\)_2(g)
Determine the stoichiometric ratios from the balanced equation: 4 moles of HCl react with 1 mole of O_2 to produce 2 moles of Cl_2.
Examine the initial mixture of reactants to identify the limiting reactant by comparing the available moles of HCl and O_2.
Calculate the maximum number of Cl_2 molecules that can be formed based on the limiting reactant using the stoichiometric ratio.
Verify the calculation by ensuring that the number of Cl_2 molecules formed does not exceed the amount predicted by the stoichiometry of the reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It allows us to determine the proportions of each substance involved in the reaction, which is essential for predicting how much product will form from given amounts of reactants.
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Stoichiometry Concept

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the yield of products, as it dictates how far the reaction can proceed.
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Molecular Ratios

Molecular ratios are derived from the coefficients of a balanced chemical equation and indicate the relative amounts of reactants and products involved in the reaction. Understanding these ratios is vital for predicting the quantities of products formed from specific amounts of reactants, particularly in determining how many molecules of Cl<sub>2</sub> can be produced.
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Related Practice
Textbook Question

Calculate the theoretical yield of the product (in moles) for each initial amount of reactants.

Ti(s) + 2 Cl2(g) → TiCl4(s)

a. 4 mol Ti, 4 mol Cl2

b. 7 mol Ti, 17 mol Cl2

c. 12.4 mol Ti, 18.8 mol Cl2

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Textbook Question

Calculate the theoretical yield of product (in moles) for each initial amount of reactants.

3 Mn(s) + 2 O2(g) → Mn3O4(s)

a. 3 mol Mn, 2 mol O2

b. 4 mol Mn, 7 mol O2

c. 27.5 mol Mn, 43.8 mol O2

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Textbook Question

Zinc sulfide reacts with oxygen according to the reaction: 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2( g) A reaction mixture initially contains 4.2 mol ZnS and 6.8 mol O2. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?

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Textbook Question

Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O2( g) → 2 Al2O3(s)

a. 1 mol Al, 1 mol O2

b. 4 mol Al, 2.6 mol O2

c. 16 mol Al, 13 mol O2

d. 7.4 mol Al, 6.5 mol O2

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1
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Textbook Question

Find the limiting reactant for each initial amount of reactants.

2 Na(s) + Br2(g) → 2 NaBr(s)

a. 2 mol Na, 2 mol Br2

b. 1.8 mol Na, 1.4 Br2

c. 2.5 mol Na, 1 mol Br2

d. 12.6 mol Na, 6.9 mol Br2

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